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    (Original post by Twinkles)
    Does NH3 never have a charge?
    Obviously it doesn't.
    Stupid Q - sorry!
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    Good luck everyone! I'm going now just remember...

    pH=-log[H+(aq)]

    haha! lets hope that is the hardest question asked
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    June 2010 6b), how do they balance the Cr2O72-?
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    (Original post by Wilzyy)
    I think Pt has a 2+ charge, then each Cl ligand has a 1- charge, the NH3 ligands have no charge. So the Pt2+ and 2CL- cancel out.
    This answer is the correct one. Pretty sure.
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    I've got a question about Potassium Manganate. How come they still call it an oxidising agent when its oxidation number increases when it reacts with other elements e.g Iron(11)? Please help?
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    do we need to learn the structure of EDTA or so u think they'll give it?
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    (Original post by Lissa-154)
    Look at the ratio of oxygens formed on the right hand side of the equation. They're in 2:1/2 right? so you divide it by 2 to get 1:1/4

    This is where the 4 comes from, so you divide the initial rate by 4
    THANK YOU!!!!!!
    phew! glad thats cleared up!
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    (Original post by Stahr1)
    I've got a question about Potassium Manganate. How come they still call it an oxidising agent when its oxidation number increases when it reacts with other elements e.g Iron(11)? Please help?
    oxidising agents cause other compounds to lose electrons whilst itself will gain electrons (reduction)
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    (Original post by Stahr1)
    I've got a question about Potassium Manganate. How come they still call it an oxidising agent when its oxidation number increases when it reacts with other elements e.g Iron(11)? Please help?
    I think it because its a self oxidising agent? MnO4 2- - - > Mn 2+
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    (Original post by Stahr1)
    I've got a question about Potassium Manganate. How come they still call it an oxidising agent when its oxidation number increases when it reacts with other elements e.g Iron(11)? Please help?
    Doesn't it decrease in oxidation number from +7 in MnO4- to +2 in Mn2+ ? So it is reduced when it reacts with Fe2+ I think.
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    hi everyone, got a question about ligands ... what are the different reactions of them? i know substitution but minds gone blank and I can't think of anything else!
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    (Original post by apo1324)
    I think it because its a self oxidising agent? MnO4 2- - - > Mn 2+
    Mn7+ +5e- -> Mn2+ electrons are gained which is reduction.
    it makes Fe2+ ->Fe3+ +e- electron is lost, which is oxidation.
    Mn7+ oxidises Fe2+, so it is an oxidizing agent.
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    (Original post by susan23)
    do we need to learn the structure of EDTA or so u think they'll give it?
    They will give it or sllow you to use symbols to represent it
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    Kc is unaffected by pressure, concentration, and catalyst.

    But K, rate constant is affected by these?:confused:
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    (Original post by Lissa-154)
    Doesn't it decrease in oxidation number from +7 in MnO4- to +2 in Mn2+ ? So it is reduced when it reacts with Fe2+ I think.
    Yea, technically its the Mn IN MnO4- that is the oxidising agent, as theoxygen go not change oxidation state
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    (Original post by Sereni)
    They will give it or sllow you to use symbols to represent it
    Ohh I hope they don't ask us to draw structure of it /ligand complex that will be worse than the Jan question on hair
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    I'm off to college to cram in the library a bit...
    So good luck everyone
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    Can we be expected to draw EDTA binding to a metal ion? :s :P
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    (Original post by jlcf)
    Kc is unaffected by pressure, concentration, and catalyst.

    But K, rate constant is affected by these?:confused:

    No, K the rate constant is also only affected by temperature
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    (Original post by jlcf)
    Kc is unaffected by pressure, concentration, and catalyst.

    But K, rate constant is affected by these?:confused:
    The rate constant is only affected by temperature, using a catalyst CHANGES the reaction and so a different rate constant is applied. Concentration changes have no effect on it also. The rate constant is linked to activation energy and temperature, for a given reaction Ea stays constant so only temperature fluctuations will cause the rate constant to vary
 
 
 
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